AP Chem

For a theoretical yield of 19 g and actual
yield of 11 g, calculate the percent yield for a
chemical reaction.
Answer in units of %.

11 g / 19 g times 100 = 57.89%
in your 2 sigfig problem, you might be expected to round off to 58%

In the reaction below, 15 g of H2S with excess
O2 produced 6 g of sulfur.
2H2S + 1O2 --> 1 S + 2H2O.

find moles, using molar mass:
15 g H2S @ 34.08 g/mol = 0.440 moles H2S

0.440 moles H2S produces 0.440 moles S

0.440 mol S @ 32.066 g/mol = 14.11 grams of Sulfur is expected

% yield =
6 g S / 14.11 g theo times 100 = 42.51 % yield

in a 2 sig fig problem this rounds to 43%

What is the percent 5)
The reaction of 8.3 grams of chlorine with
excess fluorine produced 8.6 grams of ClF3.
What percent yield of ClF3 was obtained?

using molar masses:

8.3 g Cl @ (92.45 g/mol ClF3) / (35.45 g/mol Cl) = 21.65 grams of ClF3 is expected

% yield:
8.3 / 21.65 times 100 = 38.35%

your 2 sig fig problem rounds that to 38%

  1. 👍 0
  2. 👎 0
  3. 👁 120
  1. #1 is ok.

    #2 is not. Theoretical yield is ok but actual yield is 8.6; therefore,
    (8.6/21.65)*100 = ? and round to 2 places.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    would it be: O.2576/0.7086=0.3635 0.3635 X 87.65= actual yield? A 2.30-mL sample of methane gas (density 0.112 g/cm3) was completely combusted. If the percent yield of each of the combustion products is 87.65%, calculate the

    asked by gary on October 23, 2010
  2. chemistry questions

    how do you distinquish between a limiting reactant and the excess reactant in a chemical reaction? b) how do you distinguish between the theoretical yield and actual yield in stoichiometric calculations and how does the value of

    asked by john on April 17, 2008
  3. Chemistry! Test tomorrow, pls help !

    we're given the equation: C6H6(l)+Br2(l) --> C6H5Br(l)+HBr(g) you need to prepare 50.0g pf bromobenzene and you expect no more than a 75% yield. How much benzene should you begin with if the yield is 75%. i know that % yield =

    asked by Alisha on October 4, 2012
  4. chemistry

    1) a student used 3.50 g of salicylic acid. calculate theoretical yield 2) the actual yield (from experiment) was found to be 1.50 g less than the theoretic yield (mass), calculate the percent yield 3) t

    asked by ama on July 18, 2012
  5. math

    how do you calculate theoretical yield of something? I don't know where to find the formula You go to the balanced chemical equation, and look at the mole ratio between the reactants and products. The theoretical yield is the

    asked by james on January 31, 2007
  6. Chemistry Pretest

    Fe can be prepared as 2 Al + Fe2O3 ----> 2 Fe + Al2O3. Suppose that 0.450 moles of Fe2O3 are reacted with an excess of Al. Suppose that 43.6 grams of Fe are obtained. What is the percent yield of Fe? a) 16.2% b) 60.7% c) 86.7% d)

    asked by Sarah on September 28, 2012
  7. Chemistry

    I have this question and I am pretty sure on what to use to solve it but I am just stuck. The reaction of 8 g of hydrogen and 28 g of carbon monoxide gave 16 g of methanol. What was the theoretical yield if the percent yield was

    asked by Justin on September 16, 2011
  8. Chemistry

    4 Fe + 3 O2 -> 2 Fe2O3 1. If I react 3.00g Fe and 5.75g O2, what is the theoretical yield? 2. If I’m only able to produce 3.5g, what is my percent yield? 3. If I try again, and get a 95.0% yield, what is my actual yield? For the

    asked by Anonymous on May 6, 2019
  9. chemistry

    Find te Yield of Carbon Dioxide in an Alkaseltzer Reaction. Equation: HCH3COO (Acetic Acid)+ NaHCO3 (Sodium Bicarbonate) -> NaCH3COO+ H20 (water)+ CO2 (Carbon Dioxide) So i know to find the Yield its Actual Yield / Theoretical

    asked by Sara on April 15, 2011
  10. Chemistry

    the actual yield of a reaction is 55.2g and the theoretical yield is 61.3g calculate the yield

    asked by La Jon on February 10, 2016
  11. Chemistry

    I am trying to find the theoretical yield for this lab I am working on. The steps to finidng it would be great. In my lab I took 40mls of H2O + 4g of AgNO3+ 8g of NaCL then I stirred it and filtered in a buchner funnel to be left

    asked by Gweedo8 on June 7, 2009

More Similar Questions